Question

Explain how you would convert from number of atoms of a specific element to its mass.

Short answer

To convert the number of atoms of a specific element to its mass, first, calculate the number of moles by dividing the given number of atoms by Avogadro's constant (\(6.022 \times 10^{23}\) atoms per mole). Then, find the molar mass of the element on the periodic table (in g/mol). Finally, multiply the number of moles by the molar mass to obtain the element's mass in grams.

Step-by-step solution

Find the number of moles of the element

To find the number of moles of the element, we will use Avogadro's constant, which is approximately \(6.022 \times 10^{23}\) atoms per mole. Divide the given number of atoms by Avogadro's constant: Number of moles = \(\frac{\text{Number of atoms}}{6.022 \times 10^{23}}\)

Determine the molar mass of the element

The molar mass is the mass of one mole of the element. You can find this value on the periodic table, which will provide you with the molar mass in grams per mole (g/mol). Note the molar mass of your specific element.

Calculate the mass of the element

Now, multiply the number of moles calculated in Step 1 by the molar mass determined in Step 2: Mass of the element (in grams) = Number of moles × Molar mass This will give you the mass of the specific element in grams.

Key concepts

Avogadro's Constant

When dealing with atoms and molecules, it's important to have a way to count them, as they are extremely tiny and exist in astronomically large numbers. This is where Avogadro's constant comes into play. Avogadro's constant is a fundamental scientific value that allows scientists to quantify and relate the number of particles to measurable amounts. It is defined as the number of atoms, molecules, or particles in one mole of a substance. This number is approximately \(6.022 \times 10^{23}\).

Avogadro's constant is essential in chemistry because it provides the bridge between the atomic scale and the macroscopic scale. It enables chemists to calculate how many atoms are in a given sample of a substance by converting the mass of the element to the number of atoms.

• Remember: It connects micro (atoms) to macro (grams).
• It's like knowing how many donuts are in a dozen – you can estimate the "weight" of atoms in everyday terms.

When converting atoms to moles, divide the number of atoms by Avogadro’s constant to find out how many moles you have, which is a crucial step in transforming atom counts into measurable mass.

Molar Mass

Molar mass is another key concept when converting atoms to mass. It represents the mass of one mole of a substance, typically measured in grams per mole (g/mol). Every element has a unique molar mass, which reflects the sum of the average atomic masses of all the atoms in the molecule or atom consisting of the element.

The periodic table is an indispensable tool as it provides the molar mass of each element directly below the element symbol. This value is typically expressed in atomic mass units for atomic scale representation and in grams per mole for macroscopic calculations.

• For example, the molar mass of carbon is roughly 12.01 g/mol, while for oxygen, it is about 16.00 g/mol.

To find the molar mass of a compound, simply add up the molar masses of all the elements present in the molecule or structure. Knowing the molar mass allows you to convert moles of a substance into grams, which helps in solving various chemical equations and reactions.

Atoms to Mass Conversion

Converting the number of atoms to mass involves a few systematic steps, taking advantage of Avogadro's constant and the molar mass of the element. It starts by identifying how many moles you have from a given number of atoms. Using the relationship from Avogadro's constant, you divide the number of atoms by \(6.022 \times 10^{23}\) to find your moles.

Next, you utilize the molar mass. Multiply the number of moles by the molar mass of the specific element. This calculation will give you the mass in grams.

• Example: To find the mass of 3 mol of carbon, you'd do \(3 \times 12.01 = 36.03\) grams.

These steps validate the incredible utility of moles as a unit in chemistry, as they allow us to shift from a count of atoms to a macro-scale measurement easily. The precision with these conversions enables chemists to predict the outcomes of reactions and to quantify reactants and products effectively.